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chemistry
organic chemistry

Questions and Answers of Organic Chemistry

Using Lewis symbols, diagram the reaction between magnesium and oxygen atoms to give the ionic substance MgO.
Use Lewis symbols to represent the reaction that occurs between Ca and F atoms.
Write the electron configuration for each of the following ions, and determine which ones possess noble-gas configurations: (a) Sr2+ (b) Ti2+ (c) Se2- (d) Ni2+ (e) Br- (f) Mn3+
Illustrated are four ions-A, B, X, and Y- showing their relative ionic radii. The ions shown in red carry positive charges: a2+ charge for A and a 1+ charge for B. Ions shown in blue carry negative
Write electron configurations for the following ions, and determine which have noble-gas configurations: (a) Cd2+ (b) p3- (c) Zr4+ (d) Ru3+ (e) As3- (f) Ag+
(a) Define the term lattice energy. (b) Which factors govern the magnitude of the lattice energy of an ionic compound?
NaCl and KF have the same crystal structure. The only difference between the two is the distance that separates cations and anions.(a) The lattice energies of NaCl and KF are given in Table 8.2.
The ionic substances KF, CaO, and ScN are iso-electronic (they have the same number of electrons). Examine the lattice energies for these substances in Table 8.2, and account for the trends you
(a) Does the lattice energy of an ionic solid increase or decrease (i) as the charges of the ions increase, (ii) as the sizes of the ions increase? (b) Arrange the following substances not listed in
The lattice energies of KBr and CsCl are nearly equal (Table 8.2).What can you conclude from this observation?
Explain the following trends in lattice energy: (a) NaCl > RbBr > CsBr; (b) BaO > KF (c) SrO > SrCl2
Energy is required to remove two electrons from Ca to form Ca2+ and is required to add two electrons to O to form O2-. Why, then, is CaO stable relative to the free elements?
List the individual steps used in constructing a Born-Haber cycle for the formation of BaI2 from the elements. Which of the steps would you expect to be exothermic?
Use data from Appendix C, Figure 7.9, and Figure 7.11 to calculate the lattice energy of RbCl. Is this value greater than or less than the lattice energy of NaCl? Explain.
A portion of a two-dimensional "slab" of NaCl (s) is shown here (see Figure 8.3) in which the ions are numbered.(a) Of the following types of interactions (identified by color), which are attractive
(a) Based on the lattice energies of MgCl2 and SrCl2 given in Table 8.2, what is the range of values that you would expect for the lattice energy of CaCl2?(b) Using data from Appendix C, Figure 7.9,
(a) What is meant by the term covalent bond? (b) Give three examples of covalent bonding. (c) A substance XY, formed from two different elements, boils at -33oC. Is XY likely to be a covalent or an
Which of these elements are unlikely to form covalent bonds: S, H, K, Ar, Si? Explain your choices.
Using Lewis symbols and Lewis structures, diagram the formation of SiCl4 from Si and Cl atoms.
Use Lewis symbols and Lewis structures to diagram the formation of PF3 from P and F atoms.
(a) Construct a Lewis structure for O2 in which each atom achieves an octet of electrons. (b) Explain why it is necessary to form a double bond in the Lewis structure. (c) The bond in O2 is shorter
(a) Construct a Lewis structure for hydrogen peroxide, H2O2, in which each atom achieves an octet of electrons. (b) Do you expect the O-O bond in H2O2 to be longer or shorter than the bond in O2?
(a) What is meant by the term electro negativity? (b) On the Pauling scale what is the range of electro negativity values for the elements? (c) Which element has the greatest electro negativity? (d)
(a) What is the trend in electro negativity going from left to right in a row of the periodic table? (b) How do electro negativity values generally vary going down a column in the periodic table? (c)
Using only the periodic table as your guide, select the most electronegative atom in each of the following sets: (a) Na, Mg, K, Ca; (b) P, S, As, Se; (c) Be, B, C, Si; (d) Zn, Ge, Ga, As.
The orbital diagram that follows shows the valence electrons for a 2+ ion of an element. (a) What is the element?(b) What is the electron configuration of an atom of this element?
Arrange the bonds in each of the following sets in order of increasing polarity: (a) C-F, O-F, Be-F (b) O-Cl, S-Br, C-P (c) C-S, B-F, N-O
(a) From the data in Table 8.3, calculate the effective charges on the H and Br atoms of the HBr molecule in units of the electronic charge, e.(b) Compare your answers to part (a) with those in
The iodine mono bromide molecule, IBr, has a bond length of 2.49 Å and a dipole moment of 1.21 D. (a) Which atom of the molecule is expected to have a negative charge? Explain. (b) Calculate the
In the following pairs of binary compounds determine which one is a molecular substance and which one is an ionic substance. Use the appropriate naming convention (for ionic or molecular substances)
In the following pairs of binary compounds determine which one is a molecular substance and which one is an ionic substance. Use the appropriate naming convention (for ionic or molecular substances)
Draw Lewis structures for the following: (a) SiH4, (b) CO, (c) SF2, (d) H2SO4 (H is bonded to O), (e) ClO2-, (f) NH2OH.
Write Lewis structures for the following: (a) H2CO (both H atoms are bonded to C), (b) H2O2, (c) C2F6 (contains a bond), (d) AsO33-, (e) H2SO3 (H is bonded to O), (f) C2H2
(a) When talking about atoms in a Lewis structure, what is meant by the term formal charge? (b) Does the formal charge of an atom represent the actual charge on that atom? Explain. (c) How does the
In the Lewis structure shown here, A, D, E, Q, X, and Z represent elements in the first two rows of the periodic table (H--- Ne). Identify all six elements so that the formal charges of all atoms are
(a) Write a Lewis structure for the phosphorus tri-fluoride molecule, PF3. Is the octet rule satisfied for all the atoms in your structure? (b) Determine the oxidation numbers of the P and F atoms.
Write Lewis structures that obey the octet rule for each of the following, and assign oxidation numbers and formal charges to each atom: (a) OCS, (b) SOCl2 (S is bonded to the two Cl atoms and to
For each of the following molecules or ions of sulfur and oxygen, write a single Lewis structure that obeys the octet rule, and calculate the oxidation numbers and formal charges on all the
(a)Write one or more appropriate Lewis structures for the nitrite ion, NO2- (b) With what allotrope of oxygen is it iso-electronic? (c) What would you predict for the lengths of the bonds in NO2-
Consider the format ion, HCO2-, which is the anion formed when formic acid loses an H+ ion. The H and the two O atoms are bonded to the central C atom. (a) Write one or more appropriate Lewis
Predict the ordering of the C-O bond lengths in CO, CO2, and CO32-.
Based on Lewis structures, predict the ordering of N-O bond lengths in NO+, NO2- and NO3-.
(a) Use the concept of resonance to explain why all six C-C bonds in benzene are equal in length. (b) Are the C-C bond lengths in benzene shorter than C-C single bonds? Are they shorter than C == C
Mothballs are composed of naphthalene, C10H8, a molecule of which consists of two six-member rings of carbon fused along an edge, as shown in this incomplete Lewis structure:(a) Write two complete
(a) State the octet rule. (b) Does the octet rule apply to ionic as well as to covalent compounds? Explain using examples as appropriate.
Incomplete Lewis structures for the nitrous acid molecule, HNO2, and the nitrite ion, NO2-, are shown below.(a) Complete each Lewis structure by adding electron pairs as needed.(b) Is the formal
Considering the nonmetals, what is the relationship between the group number for an element (carbon, for example, belongs to group 4A; see the periodic table on the inside front cover) and the number
The chlorine oxides, in which a chlorine atom is bonded to one or more oxygen atoms, are important molecules in the chemistry of the atmosphere. Will any of the chlorine oxides obey the octet rule?
For elements in the third row of the periodic table and beyond, the octet rule is often not obeyed. What factors are usually cited to explain this fact?
Draw the Lewis structures for each of the following ions or molecules. Identify those that do not obey the octet rule, and explain why they do not: (a) SO32-, (b) AlH3, (c) N3-, (d) CH2Cl2, (e) SbF5.
Draw the Lewis structures for each of the following molecules or ions. Which do not obey the octet rule? (a) NO, (b) BF3, (c) ICI2-, (d) OPBr3 (the P is the central atom), (e) XeF4.
In the vapor phase, BeCl2 exists as a discrete molecule. (a) Draw the Lewis structure of this molecule, using only single bonds. Does this Lewis structure satisfy the octet rule? (b) What other
(a) Describe the molecule xenon trioxide, XeO3, using four possible Lewis structures, one each with zero, one, two, or three Xe-O double bonds. (b) Do any of these resonance structures satisfy the
Consider the following statement: "For some molecules and ions, a Lewis structure that satisfies the octet rule does not lead to the lowest formal charges, and a Lewis structure that leads to the
Some chemists believe that satisfaction of the octet rule should be the top criterion for choosing the dominant Lewis structure of a molecule or ion. Other chemists believe that achieving the best
Using Table 8.4, estimate Î”H for each of the following gas-phase reactions:a.b. c.
The partial Lewis structure that follows is for a hydrocarbon molecule. In the full Lewis structure, each carbon atom satisfies the octet rule, and there are no unshared electron pairs in the
Using Table 8.4, estimate Î”H for the following gas-phase reactions:a.b. c.
Using Table 8.4, estimate Î”H for each of the following reactions:a. 2CH4 (g) + O2 †’ 2CH3OH (g)b. H2 (g) + Br2 (g) †’ 2HBr (g)c. 2H2O2 (g) †’ 2H2O (g) + O2
Use Table 8.4 to estimate the enthalpy change for each of the following reactions:a. H2C == O (g) + HCl (g) †’ H3C - O - Cl (g)b. H2O2 (g) + 2CO (g) †’ H2 (g) + CO2 (g)(c). 3H2C
Ammonia is produced directly from nitrogen and hydrogen by using the Haber process. The chemical reaction isN2 (g) + 3H2 (g) †’ 2NH3 (g)(a) Use Table 8.4 to estimate the enthalpy change for
(a) Use bond enthalpies to estimate the enthalpy change for the reaction of hydrogen with ethylene: H2 (g) + C2H4 (g) → C2H6 (g) (b) Calculate the standard enthalpy change for this reaction, using
(a) Using average bond enthalpies, predict which of the following reactions will be most exothermic: (i) C(g) + 2 F2 (g) CF4 (g) (ii) CO (g) + 3F2 → CF4 (g) + OF2 (g) (iii) CO2 (g) + 4F2 → CF4
How many elements in the periodic table are represented by a Lewis symbol with a single dot? Are all these elements in the same group? Explain.
From Equation 8.4 and the ionic radii given in Figure 7.7, calculate the potential energy of the following pairs of ions. Assume that the ions are separated by a distance equal to the sum of their
(a) Explain the following trend in lattice energy: BeH2, 3205kJ/mol; MgH2, 2791kJ/mol ; CaH2, 2410 kJ/mol ;SrH2, 2250kJ/mol; BaH2, 2121kJ/mol. (b) The lattice energy of ZnH2 is 2870kJ/mol. Based on
Consider the Lewis structure for the polyatomic oxyanion shown here, where X is an element from the third period (Na --- Ar). By changing the overall charge, n, from 1 -- to 2 --- to 3 --- we get
Based on data in Table 8.2, estimate (within 30 kJ / mol) the lattice energy for(a) LiBr,(b) CsBr,(c) CaCl2.
An ionic substance of formula MX has lattice energy of 6 × 103 kJ/mol. Is the charge on the ion M likely to be 1+, 2+ or 3+? Explain your reasoning.
From the ionic radii given in Figure 7.7, calculate the potential energy of a Ca2+ and O2- ion pair that is just touching (the magnitude of the electronic charge is given on the back inside cover).
Construct a Born-Haber cycle for the formation of the hypothetical compound NaCl2, where the sodium ion has a charge (the second ionization energy for sodium is given in Table 7.2).(a) How large
(a) How does a polar molecule differ from a non-polar one? (b) Atoms X and Y have different electro negativities. Will the diatomic molecule X-Y necessarily is polar? Explain. (c) What factors affect
For the following collection of nonmetallic elements, O, P, Te, I, B, (a) Which two would form the most polar single bond? (b) Which two would form the longest single bond? (c) Which two would be
The substance chlorine monoxide, ClO (g), is important in atmospheric processes that lead to depletion of the ozone layer. The ClO molecule has a dipole moment of 1.24 D and the Cl-O bond length is
Using the electro negativities of Br and Cl, estimate the partial charges on the atoms in the Br-Cl molecule. Using these partial charges and the atomic radii given in Figure 7.7, estimate the dipole
A major challenge in implementing the "hydrogen economy" is finding a safe, lightweight, and compact way of storing hydrogen for use as a fuel. The hydrides of light metals are attractive for
Although I3- is known, F3- is not. Using Lewis structures, explain why F3- does not form.
(a) What are valence electrons? (b) How many valence electrons does a nitrogen atom possess? (c) An atom has the electron configuration 1s22s22p63s23p2. How many valence electrons does the atom have?
Calculate the formal charge on the indicated atom in each of the following molecules or ions: (a) The central oxygen atom in O3, (b) Phosphorus in PF6-, (c) Nitrogen in NO2, (d) Iodine in ICl3, (e)
(a) Determine the formal charge on the chlorine atom in the hypochlorite ion, ClO-, and the perchlorate ion, ClO4-, using resonance structures where the Cl atom has an octet. (b) What are the
The following three Lewis structures can be drawn for N2O:(a) Using formal charges, which of these three resonance forms is likely to be the most important? (b) The N-N bond length in N2O is 1.12
(a) Triazine, C3H3N3, is like benzene except that in triazine every other C-H group is replaced by a nitrogen atom. Draw the Lewis structure(s) for the triazine molecule. (b) Estimate the
Ortho-dichlorobenzene, C6H4Cl2, is obtained when two of the adjacent hydrogen atoms in benzene are replaced with Cl atoms. A skeleton of the molecule is shown here.(a) Complete a Lewis structure for
Consider the hypothetical molecule B-A == B. How could you use an experimentally determined structure of the molecule to decide whether resonance is important in it?
An important reaction for the conversion of natural gas to other useful hydrocarbons is the conversion of methane to ethane.2CH4 (g) †’ C2H6 (g) + H2 (g)In practice, this reaction is
Two compounds are isomers if they have the same chemical formula but a different arrangement of atoms. Use Table 8.4 to Î”H estimate for each of the following gas-phase iso-merization
With reference to the "Chemistry Put to Work" box on explosives, (a) Use bond enthalpies to estimate the enthalpy change for the explosion of 1.00 g of nitroglycerin. (b) Write a balanced equation
The "plastic" explosive C-4, often used in action movies, contains the molecule cyclotrimethylenetrinitramine, which is often called RDX (for Royal Demolition eXplosive):Cyclotrimethylenetrinitramine
Write a Lewis structure for each of the following negative ions, and assign the formal negative charge to the correct atom: (a) CH3O- (b) NH2- (c) CN- (d) HCO2- (e) HCO3- (f) HC2-
Assign the proper formal charge to the colored atom in each of the following structures:(a)(b) (c) (d) (e) (f) (g) (h)
Write a condensed structural formula for the following compound.
Write each of the following condensed structural formulas as a bond-line formula:(a) (CH3)2CHCH2CH3(b) (CH3)2CHCH2CH2OH(c) (CH3)2C==CHCH2CH3(d) CH3CH2CH2CH2CH3(e) CH3CH2CH(OH)CH2CH3(f) CH2
Write a dash formula for each of the following bond-line formulas:(a)(b) (c)
Write three-dimensional (wedge-dashed wedge-line) representations for each of the following: (a) CH3Cl (b) CH2Cl2 (c) CH2BrCl (d) CH3CH2Cl
(a) Write two resonance structures for the formate ion HCO2-.(The hydrogen and oxygen atoms are bonded to the carbon.) (b) Explain what these structures predict for the carbon-oxygen bond lengths of
Write the resonance structure that would result from moving the electrons as the curved arrows indicate. Be sure to include formal charges if needed.(a)(b) (c) (d)
How many valence electrons does each of the following atoms have? (a) Na (b) Cl (c) Si (d) B (e) Ne (f) N
Add any missing unshared electron pairs (if any), then, using curved arrows to show the shifts in electrons, write the contributing resonance structures and resonance hybrid for each of the
For each set of resonance structures that follow, add a curved arrow that shows how electrons in the left formula shift to become the right formula, and designate the formula that would contribute
Which of the following alkenes can exist as c is-trans isomers? Write their structures. Build hand-held models to prove that one isomer is not superposable on the other. (a) CH2==CHCH2CH3 (b)

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